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- At what temperature is the standard molar entropy of helium equal to that of xenon at 298 K?Calculate the contribution that rotational motion makes to the molar entropy of a gas of HCl molecules at 25 °C.Suppose that the weight, W, of a configuration of N molecules in a gas of volume V is proportional to VN. Use Boltzmann's formula to deduce the change in entropy when the gas expands isothermally from Vi to Vf.
- Use mathematical software or an electronic spreadsheet to:Evaluate the change in entropy of 1.00 mol CO2(g) on expansion from 0.001 m3 to 0.010 m3 at 298 K, treated as a van der Waals gas.When a gas undergoes reversible adiabatic expansion, its entropy remains constant even though the volume increases. Explain how this can be consistent with the microscopic interpretation of entropy. Hint: consider the Maxwell Distribution of velocities.What is Isothermal Expansion of a van der Waals Gas?
- Determine an expression for V/T p, n in terms of and . Does the sign on the expression make sense in terms of what you know happens to volume as temperature changes?Define isobaric,isochoric, isenthalpic,and isothermal. Can achangein a gaseous system be isobaric, isochoric,and isothermal at the same time? Why or why not?Prove that the adiabatic free expansion of an ideal gas is spontaneous.
- Calculate the change in the entropies of the system and the surroundings, and the total change in entropy, when the volume of a sample of argon gas of mass 31.5 g at 298 K and 1.50 bar increases from 1.20 L to 4.60 L in an adiabatic reversible expansion.Calculate the value of cP at 298 K and 1 atm pressurepredicted for CH4(g) and C2H4(g) by the classical equipartition theorem. Compare the predicted results with the experimental results (see Appendix D) and calculate the percent of the measured value that arises from vibrationalmotions.Suggest a physical interpretation of the dependence of the Gibbs energy on the pressure.